Calculate the standard entropy change for the following reaction at 25 °C. 2S (s, rhombic) +3 0₂ (g) → 2 SO₂ (g) Round your answer to 4 significant digits. Note: Reference the Thermodynamic properties of pure substances tabl I J K.mol x10 X Ś

Place the following in order of  increasing molar entropy at 298 K. CO  ,   C 5H 12 ,    H 2

A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of  144.0°C  and constant total pressure. Then, he measures the reaction enthalpy  ΔH  and reaction entropy  ΔS  of the first reaction, and the reaction enthalpy  ΔH  and reaction free energy  ΔG  of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate  ΔG  for the first reaction and  ΔS  for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. →+C3H8g5O2g+3CO2g4H2Ol =ΔH−2220.kJ =ΔS−5322.JK =ΔGkJ Which is spontaneous?   this reaction     the…

Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction free energy of the following chemical reaction: C(s, graphite) + 2Cl₂ (g) → CCl4 (g) Round your answer to zero decimal places. เม kJ x10 X ? Ś

Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction entropy of the following chemical reaction: CH,OH (g)+CO (g) → HCH,CO₂ (1) Round your answer to zero decimal places. -0 K X

Calculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. MgCl₂ (s) + H₂O(1) AH;xn= V → B MgO(s) + 2 HCl(g) MacBook Air H N M 1 9 DD $10 P m kJ

0/5 Nerbs A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 85.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. do AH = -2220. kJ J AS = -6189 K C,H, (g) + 50, (g) 3Co, (g) + 4H,0(1) AG = KJ Which is spontaneous? O this reaction O the reverse reaction O neither AH = -50. kJ 0- AS =…

A chemist fills a reaction vessel with 6.88 atm hydrogen (H2) gas, 7.31 atm oxygen (O2) gas, and 1.19 atm water (H2O) gas at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: 2H2(g) + O2(g)=2H₂O(g) Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule. okJ 5 C

At constant pressure, the reaction 2A(g) → B(g) is exothermic. Which of the following statements is true for this reaction? Select one: The reaction is never spontaneous at any temperature. The reaction is spontaneous at high temperatures. It is not possible to determine the spontaneity without more information. The reaction is spontaneous at all temperatures. The reaction is spontaneous at low temperatures.

A chemicai engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 42.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. ΔΗ Ξ - 70. kJ J AS = -151. K TiCl, (g) + 2H,0(g) → Tio, (s) + 4H Cl (g) AG = || kJ Which is spontaneous? this reaction the reverse reaction neither AH = 439. kJ AS = K 4H,PO, (s) →…